Assuming that no other equilibria other than dissolution is involved, calculate the molar solubility of PbI2...
Assuming that no equilibria other than dissolution are involved, calculate the molar solubility of each of the following salts from its solubility product. (a) Ca(OH)2 Ksp = 5.0 ✕ 10−6 M (b) AgBr Ksp = 5.4 ✕ 10−13 M
13. Assuming that no equilibria other than dissolution are involved, calculate the molar solubility of each of the following from its solubility product: (a) KHC4H4O6 (b) PbI2 (C) Ag4[Fe(CN)6], a salt containing the Fe(CN)4- ion (d) Hg2I2
2. Assuming that no equilibria other than dissolution are involved, calculate the concentration of all solute species in the following solution of salts (in contact with a solution containing a common ion.) Ksp AgCl 1.6 x 10-10 AgClI(s) in 0.025 M NaCl
With respect to the dissolution of PbI2 determine: a) the reactions involved in the dissolution of PbI2 in water b) Generate the expression to determine the solubility of PbI2. c) Calculate the maximum solubility of PbI2 in water at 25 C since its ksp is 7.9 x10-9. d) Calculate the maximum solubility of PbI2 (ksp is 7.9 x10-9) at 0.500 M NaI at 25 C. e) Determine the percent difference between the solubility calculated in step d and that calculated...
Find the molar solubility of PbI2. Ksp=7.1e-9, then given the molar solubility from the previous answer, what is the solubility of PbI2, in grams per litre? Knowing this, would PbSO4 (Ksp=1.6e-8) have a higher molar solubility than PbI2? (I'm thinking PbSO4 would be higher, since the Ksp is larger?)
1/ The molar solubility of PbI2 is 1.5 x 10-3 M. a/ What is the molar concentration of iodide ion in a saturated PbI2 solution? b/ Determine the solubility constant, Ksp, for lead(II) iodide 2/ Calculate the molar solubility of PBI2 in the presence of 0.10 M NaI 3/ Compare the molar solubility given in problem 1 and the molar solubility calculated in problem 2. Explain the cause of the difference.
1. At 25 deg Celsius, the solubility product constant of PBI2 is 1.4 x 10^-8. Calculate the molar solubility in water. 2. The solubility of AgI at 25 deg Celsius is 9.1 x 10^-4 M. Calculate the Ksp of AgI at that temperature.
8. Write the ionic equation for dissolution and the solubility product (K ) expression for each of the following slightly soluble ionic compounds: (a) PbCl2 (b) Ag, S (C) Sr,(PO4)2 (d) SSO I 14. Assuming that no equilibria other than dissolution are involved, calculate the molar solubility of each of the following from its solubility product: (a) Ag, SO4 (b) PbBr2 (C) Ag! (d) CaC0, H,0
PbI2 is a sparingly soluble salt with Ksp= 1.39x10-8 What is the molar solubility of PbI2?
Answer the following questions regarding molar solubility and Ksp. a.) Calculate the molar solubility of Pbly if its Ksp value is 1.4 x 10-8. b.) Calculate the Ksp of AgCl if its molar solubility is 1.33 x 10-5 M.